Gas Laws

1
Gas Laws
2
Page 1
3
Kinetic Molecular Theory

• Is a theory that demonstrates how gases should
  behave.
• It is also called Ideal Gas Laws.

4
Kinetic Molecular Theory

• Gas particles are in random, constant,
  straight-line motion.
• Gas particles are separated by great distances
  relative to their size the volume of the gas
  particles is considered negligible.
• Gas particles have no attractive forces between
  them.
• Gas particles have collisions that may result in
  a transfer of energy between gas particles, but
  the total energy of the system remains constant.

5
Hydrogen and Helium

• Follow the Ideal Gas Law or KMT.

6
Real Gases Deviate From KMT

• The volume of gas particles is significant. Gas
  particles DO have volume.

• Gas particles DO have a force of attraction.
• The two deviations are significant under high
  pressure and low temperature (molecule are closer
  together).

7
Page 2
8
Pages 7-8
9
Page 3
10
Boyles Law

• P
• V
• Observation

11
Boyles Law

• As pressure increases, volume decrease.
• Formula P1V1 P2V2
• (Temperature and number of particles are constant)

12
Page 11

• Questions
• 3 4 6 8 - 10

Page 12

• Questions
• 1 4 6 9

13
Charles s Law

• V
• T
• Observation

14
Charles s Law

• The higher the temperature (Kelvin), the bigger
  the volume.
• Formula V1 V2
• T1(Kelvin) T2 (Kelvin)
• Pressure is Constant

15
Page 11

• Questions
• 2 7 9 - 12

Page 12

• Questions
• 3 5 7 8 - 10

16
Gay Lussacs Law

• P
• T
• Observation

17
Gay Lussacs Law

• The higher the temperature (Kelvin), the higher
  the pressure.
• Formula P1 P2
• T1(Kelvin) T2 (Kelvin)
• Volume is constant

18
Combined Gas Law

• Formula P1V1 P2V2
  (Table T)
• T1(Kelvin) T2 (Kelvin)
• Table A - STP
• May be used to solve any of the previous gas law
  problems.

19
Page 9-10
20
Page 5
21
Avagadros Hypothesis

• Equal volumes of all gases under the same
  conditions of temperature and pressure have equal
  numbers of molecules.
• Avagadros Number 6.02 x 1023
• One liter of hydrogen has the same number of
  molecules as one liter of oxygen.
• 1 mole 6.02 x 1023 particles/mol
• 1 mole of a gas occupies 22.4 liters at STP

22
Page 6